Atomic Structure

1. 4

2. 3

3. 1

4. 2

5. 1

6. 2

7. 4

8. 3

9. 53.3%

10. 2

11. 1

12. 2

13. 2

14. 3

15. 3

16. 2-7-4

17. 15 neutrons

18. 28.09 amu

19. 6.47%

20. 1

21. 2

22. 3

23. 2

24. 3

25. 1

26. 4

27. 2

28. 2-7-5

29. # of protons; # of neutrons; # of electrons in inner occupied principal energy levels

30. 23

31. Lewis structures show valence electrons only; the valence electrons are the only electrons involved in the formation of chemical bonds.

 

Periodic Table

1.  1

2. 2

3. 1

4. four

5. 1 valence electron

6. any number less than 64 degrees

7. D

8. 3

9. 3

10. 4

11. 3

12. 3

13. 1

14. 1

15. Uut with three dots around the symbol

16. +113

17. thallium, indium, gallium, aluminum

18. 4

19. 1

20. 4

21. 4

22. 4

23. Group one metals react violently with water to form Na+ ions

 

Bonding

1.  4

2. 2

3. 4

4. 1

5. 3

6. 2

7. 53.3%

8. 2KClO3 -> 2KCl + 3O2

9. The electronegativity difference between P-Cl is greater than the electronegativity difference for P-S.

10. 2

11. 4

12. 3

13. 3

14. 3 sig figs

15. 35.7%

16. To remove all the water from the hydrate to get the mass of only the anhydrous salt at the end of the experiment

17. 3

18. 4

19. 3

20. C4H9

 

Matter

For the matter section, anything involving the calculation of heat (q) will not be on the midterm. However, you still need to understand the concepts of the different phases of matter and kinetic/potential energy.

1.  3

2. 4

3. 1

4. 1

5. 2

skip 6

7. 4

skip 8

9. 3

skip 10-15

16. 0.89 g/L

17. Draw at least six molecules spread out on the entire bottom of the container. Draw at least six gas molecules floating above the liquid with adequate spacing between each gas molecule.

18. 1

19. 2

skip 20

21. 2

22. 3

23. 4

24. 3

skip 25-35

36. 14.2%

27. candle melted

28. candle is burning (flame = energy change)